Consider a galvanic electrochemical cell constructed using Cr/Cr³⁺ and Zn/Zn²⁺ at 25 °C. The following half-reactions...
Consider a galvanic electrochemical cell constructed using Cr/Cr³⁺ and Zn/Zn²⁺ at 25 °C. The following half-reactions are provided for each metal: Cr³⁺(aq) + 3 e⁻ → Cr(s) E°red = -0.744 V Zn²⁺(aq) + 2 e⁻ → Zn(s) E°red = -0.763 V
which half reaction takes place at the anode
which is the standar cell potential
write the balance equation for the overall reaction in acidic sol
What is the cell potential for this cell at 25 °C when [Zn²⁺] = 0.0343 M and [Cr³⁺] = 0.1756 M?
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Consider a galvanic electrochemical cell constructed using
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Please help me solve this
An electrochemical reaction occurring in a galvanic cell is expressed using the standard cell notation: Zn(s) Zn2+ (aq) || Ag (aq) | Ag(s) The standard reduction potentials for the half-cell reactions are as follows: Zn2+(aq) + 2e_? Zn(s) E o=-0.76 V Ag (a)eAg(s) E +0.80 V Which of the following statements is correct regarding this electrochemical cell? A. Agt is reduced at the cathode; Zn is oxidized at the anode. B. Edell = +1.56 V...
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